"A chemical bond is a lasting attraction between atoms or ions that enables the formation of molecules, crystals, and other structures."
The process by which atoms or molecules form chemical bonds and become united into compounds.
Valence Electrons: The outermost electrons of an atom that participate in chemical bonding.
Lewis Structures: A method to represent the valence electrons of a molecule as dots or lines.
Ionic Bond: A chemical bond formed by the transfer of electrons between atoms, leading to the formation of oppositely charged ions.
Covalent Bond: A chemical bond formed by the sharing of electrons between atoms.
Metallic Bond: A type of bonding in metals where the valence electrons are delocalized, allowing for high conductivity and malleability.
Hybridization: The mixing of atomic orbitals to form new hybrid orbitals that better explain the properties of molecules.
Molecular Orbital Theory: A theory that describes the molecular orbitals formed by the overlapping of atomic orbitals in a molecule.
Dipole Moments: A measure of the polarity of a molecule formed due to an unequal distribution of electrons.
Formal Charge: A method to calculate the charge on an atom in a molecule.
VSEPR Theory: A theory that describes the shape of a molecule based on the repulsion between electron pairs in the valence shell of an atom.
Molecular Polarity: The overall polarity of a molecule based on the polarity of its bonds and the molecular shape.
Intermolecular Forces: Forces between molecules that affect physical properties such as boiling point and solubility. These include London dispersion forces, dipole-dipole forces, and hydrogen bonding.
Valence Bond Theory: A theory that describes chemical bonding as the overlap of atomic orbitals to allow for the formation of shared electron pairs.
Chemical Reactivity: How chemical bonding affects the ability of molecules to undergo chemical reactions, including factors such as bond strength, bond length, and electronegativity.
Resonance Structures: Multiple valid Lewis structures for a molecule that have the same arrangement of atoms but different arrangements of electrons.
Covalent bonding: This occurs when atoms share electrons to form a stable molecule. Covalent bonds can be either polar or nonpolar.
Ionic bonding: This occurs when a positively charged ion, called a cation, and a negatively charged ion, called an anion, are attracted to each other through an electrostatic force.
Metallic bonding: This occurs when metal atoms share their valence electrons within a lattice structure, resulting in a unique set of physical properties such as electrical conductivity and ductility.
Hydrogen bonding: This is a type of intermolecular force in which a hydrogen atom is covalently bonded to one electronegative atom and is also weakly bonded to another electronegative atom.
Coordinative bonding: This occurs when one atom donates a pair of electrons to another atom, creating a shared pair of electrons called a coordination bond.
Van der Waals bonding: This is a weak intermolecular force that arises from temporary dipoles in nonpolar molecules.
Dipole-dipole interactions: This occurs when two polar molecules interact with each other through electrostatic forces between their respective dipoles.
π-bonding: This occurs when p-orbitals overlap, resulting in the formation of π-bonds that are characteristic of double and triple bonds.
Metallic-covalent bonding: This is a type of bonding that is found in alloys, where metal atoms share their valence electrons with other metal atoms and also form covalent bonds with nonmetal atoms.
Halogen bonding: This occurs when halogen atoms interact with other molecules through their partial negative charges, resulting in a type of chemical interaction that is similar to hydrogen bonding.
Charge-transfer bonding: This occurs when electrons are transferred from one atom to another in a chemical reaction, producing an ionic compound.
Steric effects: This is a type of noncovalent interaction that arises from the repulsion or attraction of atoms due to the spatial arrangement of electrons within a molecule.
Three-center bonding: This occurs when three atoms share electrons to form a stable molecule or ion.
Cuprate bonding: This is a type of bonding that is characteristic of copper-containing compounds, where the copper atoms form chains or planes that interact through delocalized electrons.
Resonance: This is a phenomenon that occurs when a molecule has multiple equivalent Lewis structures, which are the same in energy and contribute to the overall stability of the molecule.
Charge-induced dipole interactions: This occurs when a charged molecule induces a dipole in a nearby atom or molecule, resulting in a type of temporary bonding.
"The bond may result from the electrostatic force between oppositely charged ions as in ionic bonds."
"The bond may result from...the sharing of electrons as in covalent bonds."
"There are 'strong bonds' or 'primary bonds' such as covalent, ionic and metallic bonds."
"There are 'weak bonds' or 'secondary bonds' such as dipole-dipole interactions, the London dispersion force, and hydrogen bonding."
"The negatively charged electrons surrounding the nucleus and the positively charged protons within a nucleus attract each other."
"Electrons shared between two nuclei will be attracted to both of them."
"Constructive quantum mechanical wavefunction interference stabilizes the paired nuclei."
"Bonded nuclei maintain an optimal distance (the bond distance) balancing attractive and repulsive effects explained quantitatively by quantum theory."
"The atoms in molecules, crystals, metals, and other forms of matter are held together by chemical bonds."
"All bonds can be described by quantum theory, but, in practice, simplified rules and other theories allow chemists to predict the strength, directionality, and polarity of bonds."
"The octet rule and VSEPR theory are examples."
"More sophisticated theories are valence bond theory, which includes orbital hybridization and resonance."
"More sophisticated theories...include molecular orbital theory, which includes the linear combination of atomic orbitals and ligand field theory."
"Electrostatics are used to describe bond polarities and the effects they have on chemical substances."
"The strength of chemical bonds varies considerably."
"The octet rule is an example [of a theory] that allows chemists to predict the strength, directionality, and polarity of bonds."
"The VSEPR theory is an example [of a theory] that allows chemists to predict the strength, directionality, and polarity of bonds."
"Orbital hybridization is a component of valence bond theory."
"Ligand field theory is a component of molecular orbital theory."